O ATOMS, IONS AND MOLECULESUnderstanding the difference between a molecular and empiric...What are the molecular and empirical chemical formulas of a compound made up of these molecules?H H H HHÖ-C-C=C—C—Ö-HescHmolecular formula: 00empirical formula:Explanation1HFICheck#80F3The lines stand for chemical bonds between the atoms. You can ignore the dots -- they represent "lone pairs" andyou'll learn about them later.X$F45%F5MacBook AirA&F7©2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center AccessibilityDI10/3FBF10C+F12

Molecular formula -> A chemical formula that gives the total number of atoms of each element in…

= O ATOMS, IONS AND MOLECULES Understanding the difference between a molecular and empiric... What are the molecular and empirical chemical formulas of a compound made up of these molecules? H H H H H- C H C C C molecular formula: empirical formula: Explanation H 0 Check 0 H The lines stand for chemical bonds between the atoms. You can ignore the dots -- they represent "lone pairs" and you'll learn about them later. X 0 0/3 S

= O ATOMS, IONS AND MOLECULES Understanding the difference between a molecular and empiric... What are the molecular and empirical chemical formulas of a compound made up of these molecules? H H H H H- C H C C C molecular formula: empirical formula: Explanation H 0 Check 0 H The lines stand for chemical bonds between the atoms. You can ignore the dots -- they represent "lone pairs" and you'll learn about them later. X 0 0/3 S

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 94AP: The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six...

See similar textbooks

Similar questions

The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.
A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.
The percent ionic character of a bond can be approximated by the formula 16+3.52 , where is the magnitude of the difference in the electronegativities of the atoms (see Fig. 3.18). Calculate the percent ionic character of HF, HCl, HBr, HI, and CsF, and compare the results with those in Table 3.7.
Estimate the percent ionic character of the bond in each of the following species. All the species are unstable or reactive under ordinary laboratory conditions, but they can be observed in interstellar space.
For each pair of bonds, predict which is the shorter. (a) SiN or PO (b) SiO or CO (c) CF or CBr (d) The C=C or the CN bond in acrylonitrile, H2C=CHCN
Given the bonds C N, C H, C Br, and S O, (a) which atom in each is the more electronegative? (b) which of these bonds is the most polar?
Draw the correc (best) Lewis structure (LS) for the ionic compound K2SeO3 (on looose leaf paper--NOT TO BE SUBMITTED) and then answer the following questions.(NOTE: Use the cardinal numbers 0, 1, 2, 3, and so on for any quantity required)a) What charge does the K ion have in this compound? (give size & sign of charge: e.g., 1+, 2-, etc.) b) What charge does the SeO3 ion have in this compound? (give size & sign of charge: e.g., 1+, 2-, etc.) c) How many lines, if any, attach each K ion to the SeO3 ion? d) How many valence electrons does the SeO3 ion (alone) have? e) How many single bonds does the LS of the SeO3 ion have? f) What is the number of lone electron pairs in the LS of the SeO3 ion?
A new compound is made that has a C—C bond length of1.15 Å. Is this bond likely to be a single, double, or tripleC—C bond?
Given the following molecules and/or ions, characterize them according to the formatshown in the table below. The central atom of the molecule/ion is shown in boldface.The central atom or molecules marked with an asterisk (*) do not obey the octet rule.a. BF3b. NH3c. BeCl2d. PCl5*e. OF2f. SF4*g. SF6*h. XeF2*i. SnCl4j. H3O+ Set up your own table to the following formatColumn CharacteristicsA Bonding electronsB Sigma-bondsC Nonbonding electron pairsD Hybrid orbitals havingnonbonding electron pairsE Hybrid orbitals used F 3-D structureG Polar (P) or nonpolar (NP) molecule or ion lewis structure A B C D E F G
The dipole moment (μ�) of HBrHBr (a polar covalent molecule) is 0.831D0.831D (debye), and its percent ionic character is 12.3 %% . Estimate the bond length of the H−BrH−Br bond in picometers. Note that 1 D=3.34×10−30 C⋅m1 D=3.34×10−30 C⋅m and in a bond with 100%% ionic character, Q=1.6×10−19 C�=1.6×10−19 C. Express your answer to two significant figures and include the appropriate units.
If given H2, CH4, CH3 CH3, NH3 and H2O in which one of the following pre dominantly covalent molecule is the departure from equal sharing of the bonding electrons greatest and why?
Determine the molecular structure of the following compound (C4H10O) using the data below Please show how you determined the structure